Consider the reaction 2HCl(g)→ H₂(g)+ Cl₂(g); ΔH = 185 kJ Which of the following statements is false? A)The reaction is endothermic. B)HCl(g)has a negative enthalpy of formation. C)The products have more enthalpy than the reactants. D)The HCl bond is longer than either the H₂ bond or the Cl₂ bond. E)The bond order of each of the products is one.

Question

Quizplus · Accepted Answer

According to the reaction, the products have more enthalpy than the reactants, which indicates that the reaction is endothermic. HCl(g) has a negative enthalpy of formation because it is an exothermic compound, which releases energy when formed. The bond order of each of the products is one because they are both diatomic molecules. However, the HCl bond is shorter than either the H₂ bond or the Cl₂ bond because HCl is a smaller molecule than either of the products. Therefore, statement D is false.

Consider the Reaction 2HCl(g)→ H2(g)+ Cl2(g); ΔH = 185 KJ

Consider the Reaction 2HCl(g)→ H₂(g)+ Cl₂(g); ΔH = 185 KJ